a) How much lime and what volume of CO2 at NTP will be obtained from 10 kg of limestone?
b) How much ferrous sulphide will be required to obtain 1.12 g of gas at NTP by chemical reaction between ferrous sulphide and very dil.Sulphuric acid?
5.79 g
a) To answer this question, we need to know the chemical equation for the reaction between limestone and CO2. Assuming it undergoes complete decomposition, the reaction can be represented as follows:
CaCO3 (limestone) → CaO (lime) + CO2
The molar mass of CaCO3 is 100.09 g/mol, and the molar mass of CO2 is 44.01 g/mol. From this, we can calculate the number of moles of CaCO3 in 10 kg:
Number of moles of CaCO3 = (10 kg / 100.09 g/mol) = 99.93 mol
Since the reaction is 1:1, the number of moles of lime (CaO) and CO2 produced will also be 99.93 mol. Now, we can calculate the mass and volume of CO2 at NTP.
Mass of CO2 = Number of moles of CO2 × Molar mass of CO2
= 99.93 mol × 44.01 g/mol
= 4397.1 g
The molar volume of any ideal gas at NTP (Normal Temperature and Pressure) is approximately 22.4 L/mol. Therefore, we can calculate the volume of CO2:
Volume of CO2 = Number of moles of CO2 × Molar volume at NTP
= 99.93 mol × 22.4 L/mol
= 2238.43 L
b) To determine the amount of ferrous sulphide (FeS) needed, we need the chemical equation for the reaction between FeS and sulphuric acid. The reaction can be represented as follows:
FeS (ferrous sulphide) + H2SO4 (sulphuric acid) → FeSO4 (ferrous sulfate) + H2S (gas)
Based on the equation, we can see that 1 mole of FeS reacts to produce 1 mole of H2S gas. Therefore, the number of moles of FeS required can be calculated as the same number of moles of H2S produced.
Number of moles of FeS = Number of moles of H2S = (1.12 g / molar mass of H2S)
The molar mass of H2S is 34.08 g/mol. Substituting the value, we get:
Number of moles of FeS = 1.12 g / 34.08 g/mol
≈ 0.0329 mol
So, approximately 0.0329 moles of ferrous sulphide will be required to obtain 1.12 g of gas at NTP.
a) To determine the amount of lime and volume of CO2 obtained from 10 kg of limestone, we need to consider the chemical reaction involved and the stoichiometry.
The chemical equation for the reaction between limestone (calcium carbonate, CaCO3) and heat is:
CaCO3 (s) → CaO (s) + CO2 (g)
From this equation, we can see that one mole of calcium carbonate will produce one mole of calcium oxide (lime), and one mole of carbon dioxide.
1 mole of CaCO3 = 100 g (molar mass of CaCO3)
So, 10 kg (or 10,000 g) of limestone would be equal to:
10,000 g / 100 g/mol = 100 moles of CaCO3
Therefore, from 100 moles of CaCO3, we can expect to obtain 100 moles of CaO (lime) and 100 moles of CO2.
To determine the volume of CO2 at NTP (Normal Temperature and Pressure), we need to consider the ideal gas law, which states:
PV = nRT
Where:
P = pressure (at NTP, P = 1 atm)
V = volume
n = number of moles
R = ideal gas constant (0.0821 L•atm/(mol•K))
T = temperature (at NTP, T = 273.15 K)
For CO2 at NTP, we can assume that the volume is equal to the number of moles (n) in liters.
So, the volume of CO2 obtained from 10 kg of limestone would be:
V = n = 100 moles
b) To determine the amount of ferrous sulphide required to obtain 1.12 g of gas at NTP, we need to consider the chemical reaction and stoichiometry involved.
The chemical equation for the reaction between ferrous sulphide (FeS) and sulphuric acid (H2SO4) is:
FeS (s) + H2SO4 (aq) → FeSO4 (aq) + H2S (g)
From this equation, we see that one mole of ferrous sulphide reacts with one mole of sulphuric acid to produce one mole of hydrogen sulfide (H2S) gas.
To find the number of moles of H2S gas produced:
Mass of H2S = 1.12 g
Molar mass of H2S = 2 g/mol + 32 g/mol = 34 g/mol
Number of moles of H2S = Mass of H2S / Molar mass of H2S
Number of moles of H2S = 1.12 g / 34 g/mol
Once we know the number of moles of H2S gas, we can use the stoichiometry of the equation to determine the number of moles of ferrous sulphide required. From the equation, we see that:
1 mole of FeS produces 1 mole of H2S
Therefore, the number of moles of FeS = Number of moles of H2S
Now, you can calculate the amount of ferrous sulphide required.